In a displacement reaction, what occurs when aqueous chlorine is added to a solution of potassium bromide?

Chlorine displaces bromine because it has a smaller atomic radius and a stronger attraction for an incoming electron.

Bromine displaces chlorine because it is more reactive further down Group 7.

No reaction occurs because bromine is a liquid and chlorine is a gas at room temperature.

A white precipitate of potassium chloride forms while the solution remains colorless.

Why are Group 0 elements, such as Neon and Argon, chemically inert in almost all standard conditions?

They possess a full outer shell of electrons, meaning they have no tendency to gain, lose, or share electrons.

Their boiling points are extremely low, so they do not have enough thermal energy to form covalent bonds.

They exist only as monatomic gases, which prevents them from colliding with other elements effectively.

The electrostatic attraction between the nucleus and the outer electrons is so strong that no electrons can be shared.

Mendeleev's periodic table was widely accepted by the scientific community primarily because:

He left gaps for undiscovered elements and accurately predicted the properties of those elements based on periodic trends.

He was the first to arrange all known elements strictly by their atomic number.

He correctly identified that all noble gases belonged in a single group at the start of the table.

He organized elements into blocks based on their $s$, $p$, $d$, and $f$ orbitals.

Which statement accurately compares the physical properties of Transition Metals to those of Group 1 Alkali Metals?

Transition metals generally have higher densities and higher melting points than Group 1 metals.

Group 1 metals are harder and more resistant to corrosion than Transition metals.

Transition metals react more vigorously with water to produce hydrogen gas.

Group 1 compounds are typically colored, whereas Transition metal compounds are usually white.

Across Period 3 of the periodic table, from Sodium ($Na$) to Argon ($Ar$), how does the atomic radius change?

The atomic radius decreases because the increasing nuclear charge pulls the electron shells closer to the nucleus.

The atomic radius increases because more electrons are added to the shells, causing them to expand.

The atomic radius stays the same because all elements in Period 3 have three occupied electron shells.

The atomic radius increases because the mass of the atom increases with the addition of neutrons.

What are the products of the reaction between Lithium and water?

$\text{LiOH}$ and $\text{H}_{2}$

$\text{Li}_{2}\text{O}$ and $\text{H}_{2}$

$\text{LiH}$ and $\text{O}_{2}$

$\text{LiOH}$ and $\text{O}_{2}$

Identify the correct subshell electron configuration for Calcium (atomic number 20) provided in the extended periodic table data.

$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2}$

$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{2}$

$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4p^{2}$

How does the boiling point of the Noble Gases (Group 0) change down the group?

It increases because the atoms get larger, leading to stronger intermolecular forces between them.

It decreases because the atoms become heavier and move more slowly.

It stays the same because all noble gases have full outer shells and no polarity.

It increases because the reactivity increases down the group.

What occurs to the 'metallic character' of elements as you move from left to right across a period?

It decreases because elements are less likely to lose electrons and more likely to gain them.

It increases because there are more electrons available in the outer shell to form metallic bonds.

It remains constant until you reach the zigzag line.

It increases because the atomic number is increasing.

Why did Mendeleev occasionally switch the order of elements, such as Tellurium and Iodine, in his table?

To ensure that elements with similar chemical properties were grouped together.

Because he realized the atomic mass measurements were always incorrect.

To make room for the noble gases he had already discovered.

Because Iodine has a higher atomic number than Tellurium.

What is the trend for melting points in Group 1 metals as you move down from Lithium to Caesium?

The melting point remains constant because they all have one outer electron.

The melting point increases then decreases starting from Potassium.

What is the primary difference between the arrangement of the modern periodic table and Mendeleev's periodic table?

The modern table is arranged by atomic number, while Mendeleev used atomic mass.

The modern table includes transition metals, whereas Mendeleev's did not.

Mendeleev's table was organized by color, while the modern table is not.

The modern table is arranged alphabetically by the element names.

What observation would be expected when Potassium is added to water, which distinguishes it from the reaction of Sodium?

It reacts more vigorously and produces a lilac flame.

It sinks to the bottom and reacts slowly with bubbles.

It turns the water red instead of alkaline.

It forms a solid white precipitate immediately.

Which of the following is a common property of Transition Metal compounds?

They often form brightly colored compounds.

They always react explosively with cold water.

They are typically gaseous at room temperature.

They cannot act as catalysts in chemical reactions.

Why does the reactivity of Group 7 elements decrease as the atomic number increases?

The outer shell is further from the nucleus, so the attraction for an incoming electron is weaker.

The atoms become more metallic further down the group.

The melting point increases, making the atoms less mobile.

They have more outer electrons that repel incoming electrons.

What determines the Period an element belongs to in the periodic table?

The number of occupied electron shells in the atom.

The number of electrons in the outer shell.

The total number of neutrons in the nucleus.

The state of matter at room temperature.

In the context of periodic trends, what is meant by 'shielding'?

The reduction in attraction between the nucleus and outer electrons caused by inner electron shells.

The protective layer of oxide that forms on the surface of reactive metals.

The use of noble gases to provide an unreactive atmosphere for industrial reactions.

The physical distance between the nucleus and the valence shell.

Which of the following describes the trend in density for Group 1 metals?

Density generally increases as you move down the group.

Density decreases because the atoms get much larger.

All Group 1 metals have the same density because they are all in the same group.

Density decreases then increases starting from Potassium.

GCSE Chemistry revision

GCSE Periodic Table: Complete Revision Guide for AQA and Edexcel

Interactive revision

What Is the Periodic Table?

This GCSE periodic table revision guide covers groups, periods, trends and electronic structure for AQA and Edexcel, with an interactive table, exam-style questions and a free PDF download. The aim is to use patterns rather than memorise every element. AQA and Edexcel students need to read atomic number, groups, periods, metals, non-metals and electronic structure from the table. This AQA GCSE periodic table guide gives you a quick route: inspect an element, check its group and period, then link that evidence to properties and exam-style explanations. If you need the electron-shell basics first, start with our GCSE atomic structure revision.

Hydrogen, atomic number 1, Group 1, period 1, electron configuration 1 (GCSE shell model).
Helium, atomic number 2, Group 0, period 1, electron configuration 2 (GCSE shell model).
Lithium, atomic number 3, Group 1, period 2, electron configuration 2,1 (GCSE shell model).
Beryllium, atomic number 4, Group 2, period 2, electron configuration 2,2 (GCSE shell model).
Boron, atomic number 5, Group 13, period 2, electron configuration 2,3 (GCSE shell model).
Carbon, atomic number 6, Group 14, period 2, electron configuration 2,4 (GCSE shell model).
Nitrogen, atomic number 7, Group 15, period 2, electron configuration 2,5 (GCSE shell model).
Oxygen, atomic number 8, Group 16, period 2, electron configuration 2,6 (GCSE shell model).
Fluorine, atomic number 9, Group 7, period 2, electron configuration 2,7 (GCSE shell model).
Neon, atomic number 10, Group 0, period 2, electron configuration 2,8 (GCSE shell model).
Sodium, atomic number 11, Group 1, period 3, electron configuration 2,8,1 (GCSE shell model).
Magnesium, atomic number 12, Group 2, period 3, electron configuration 2,8,2 (GCSE shell model).
Aluminium, atomic number 13, Group 13, period 3, electron configuration 2,8,3 (GCSE shell model).
Silicon, atomic number 14, Group 14, period 3, electron configuration 2,8,4 (GCSE shell model).
Phosphorus, atomic number 15, Group 15, period 3, electron configuration 2,8,5 (GCSE shell model).
Sulfur, atomic number 16, Group 16, period 3, electron configuration 2,8,6 (GCSE shell model).
Chlorine, atomic number 17, Group 7, period 3, electron configuration 2,8,7 (GCSE shell model).
Argon, atomic number 18, Group 0, period 3, electron configuration 2,8,8 (GCSE shell model).
Potassium, atomic number 19, Group 1, period 4, electron configuration 2,8,8,1 (GCSE shell model).
Calcium, atomic number 20, Group 2, period 4, electron configuration 2,8,8,2 (GCSE shell model).
Scandium, atomic number 21, Group 3, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d1.
Titanium, atomic number 22, Group 4, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d2.
Vanadium, atomic number 23, Group 5, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d3.
Chromium, atomic number 24, Group 6, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d4.
Manganese, atomic number 25, Group 7, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d5.
Iron, atomic number 26, Group 8, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d6.
Cobalt, atomic number 27, Group 9, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d7.
Nickel, atomic number 28, Group 10, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d8.
Copper, atomic number 29, Group 11, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d9.
Zinc, atomic number 30, Group 12, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10.
Gallium, atomic number 31, Group 13, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1.
Germanium, atomic number 32, Group 14, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2.
Arsenic, atomic number 33, Group 15, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3.
Selenium, atomic number 34, Group 16, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4.
Bromine, atomic number 35, Group 7, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5.
Krypton, atomic number 36, Group 0, period 4, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6.
Rubidium, atomic number 37, Group 1, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1.
Strontium, atomic number 38, Group 2, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2.
Yttrium, atomic number 39, Group 3, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d1.
Zirconium, atomic number 40, Group 4, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d2.
Niobium, atomic number 41, Group 5, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d3.
Molybdenum, atomic number 42, Group 6, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d4.
Technetium, atomic number 43, Group 7, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d5.
Ruthenium, atomic number 44, Group 8, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d6.
Rhodium, atomic number 45, Group 9, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d7.
Palladium, atomic number 46, Group 10, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d8.
Silver, atomic number 47, Group 11, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9.
Cadmium, atomic number 48, Group 12, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10.
Indium, atomic number 49, Group 13, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p1.
Tin, atomic number 50, Group 14, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p2.
Antimony, atomic number 51, Group 15, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p3.
Tellurium, atomic number 52, Group 16, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p4.
Iodine, atomic number 53, Group 7, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5.
Xenon, atomic number 54, Group 0, period 5, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6.
Caesium, atomic number 55, Group 1, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s1.
Barium, atomic number 56, Group 2, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2.
Lanthanum, atomic number 57, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f1.
Cerium, atomic number 58, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f2.
Praseodymium, atomic number 59, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f3.
Neodymium, atomic number 60, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f4.
Promethium, atomic number 61, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f5.
Samarium, atomic number 62, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f6.
Europium, atomic number 63, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f7.
Gadolinium, atomic number 64, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f8.
Terbium, atomic number 65, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f9.
Dysprosium, atomic number 66, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f10.
Holmium, atomic number 67, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f11.
Erbium, atomic number 68, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f12.
Thulium, atomic number 69, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f13.
Ytterbium, atomic number 70, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14.
Lutetium, atomic number 71, Lanthanide, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d1.
Hafnium, atomic number 72, Group 4, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d2.
Tantalum, atomic number 73, Group 5, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d3.
Tungsten, atomic number 74, Group 6, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d4.
Rhenium, atomic number 75, Group 7, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d5.
Osmium, atomic number 76, Group 8, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d6.
Iridium, atomic number 77, Group 9, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d7.
Platinum, atomic number 78, Group 10, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d8.
Gold, atomic number 79, Group 11, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d9.
Mercury, atomic number 80, Group 12, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10.
Thallium, atomic number 81, Group 13, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p1.
Lead, atomic number 82, Group 14, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p2.
Bismuth, atomic number 83, Group 15, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p3.
Polonium, atomic number 84, Group 16, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p4.
Astatine, atomic number 85, Group 7, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p5.
Radon, atomic number 86, Group 0, period 6, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6.
Francium, atomic number 87, Group 1, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s1.
Radium, atomic number 88, Group 2, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2.
Actinium, atomic number 89, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f1.
Thorium, atomic number 90, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f2.
Protactinium, atomic number 91, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f3.
Uranium, atomic number 92, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f4.
Neptunium, atomic number 93, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f5.
Plutonium, atomic number 94, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f6.
Americium, atomic number 95, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f7.
Curium, atomic number 96, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f8.
Berkelium, atomic number 97, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f9.
Californium, atomic number 98, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f10.
Einsteinium, atomic number 99, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f11.
Fermium, atomic number 100, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f12.
Mendelevium, atomic number 101, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f13.
Nobelium, atomic number 102, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14.
Lawrencium, atomic number 103, Actinide, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d1.
Rutherfordium, atomic number 104, Group 4, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d2.
Dubnium, atomic number 105, Group 5, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d3.
Seaborgium, atomic number 106, Group 6, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d4.
Bohrium, atomic number 107, Group 7, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d5.
Hassium, atomic number 108, Group 8, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d6.
Meitnerium, atomic number 109, Group 9, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d7.
Darmstadtium, atomic number 110, Group 10, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d8.
Roentgenium, atomic number 111, Group 11, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d9.
Copernicium, atomic number 112, Group 12, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10.
Nihonium, atomic number 113, Group 13, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p1.
Flerovium, atomic number 114, Group 14, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p2.
Moscovium, atomic number 115, Group 15, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p3.
Livermorium, atomic number 116, Group 16, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p4.
Tennessine, atomic number 117, Group 7, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p5.
Oganesson, atomic number 118, Group 0, period 7, electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6.

Key to colours

Group 1 alkali metals

Group 2 alkaline earth metals

Transition metals

Other metals

Metalloids

Non-metals

Group 7 halogens

Group 0 noble gases

Lanthanides

Actinides

Download the GCSE periodic table PDF

Keep a printable periodic table beside your revision notes while you practise groups, periods, atomic number and electronic structure questions.

Download GCSE periodic table PDF

Groups and Periods — What You Need to Know (AQA spec 1.2)

Note: AQA GCSE Chemistry officially lists this content under 4.1.2 The periodic table, while many revision maps and topic checklists refer to the same area as Topic 1.2 Periodic Table.

Periods

Rows across the table

Atomic number increases from left to right. Elements in the same period have the same number of occupied electron shells.

Groups

Columns down the table

Elements in the same group have the same number of outer electrons, so they usually have similar chemical properties.

Metals / non-metals

Zigzag boundary

Metals are mostly on the left and lower parts of the table. Non-metals are mostly on the right and upper parts.

Test yourself on Groups and Periods

Use a QuizLuna chemistry quiz to check whether you can move from a position in the table to the correct group, period, outer electrons and likely properties.

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Group 1 — Alkali Metals (AQA & Edexcel)

Group 1 contains lithium, sodium, potassium, rubidium and caesium. These alkali metals have one outer electron and become more reactive down the group. Their density generally increases down the group, while melting point decreases.

The classic GCSE reaction is metal + water → metal hydroxide + hydrogen. Sodium floats, fizzes and moves on water; potassium reacts more vigorously and may burn with a lilac flame.

Memory note: The further down Group 1, the more reactive. This is a standard AQA and Edexcel exam explanation because the outer electron is further from the nucleus and easier to lose. Practise the pattern with the Group 1 alkali metals quiz.

Group 1 Metals GCSE Quiz

Practise trend explanations, observations with water and word equations for alkali metals.

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Group 7 Halogens GCSE: Reactivity and Displacement

Group 7 contains fluorine, chlorine, bromine and iodine. Reactivity decreases down the group, which is the opposite direction from Group 1. Halogen atoms have seven outer electrons and react by gaining one electron.

Displacement reactions are common GCSE exam questions: a more reactive halogen displaces a less reactive halogen from its compound. Chlorine can displace bromine or iodine, but iodine cannot displace chlorine. Use the Group 7 halogens quiz to test this trend.

Colours and physical states

Fluorine: pale yellow gas
Chlorine: green gas
Bromine: orange liquid
Iodine: grey solid

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Group 0 Noble Gases GCSE

Group 0 contains helium, neon, argon, krypton, xenon and radon. These elements are called noble gases because they are very unreactive. In GCSE answers, the reason matters: their atoms have full outer electron shells, so they do not need to gain, lose or share electrons.

Boiling points increase down Group 0 because the atoms get larger and the forces between atoms become stronger. AQA and Edexcel questions often ask students to explain why noble gases are used in lighting, balloons or inert atmospheres.

Common exam wording

Avoid writing only “stable”. A stronger answer says: noble gases have full outer shells, so they are unreactive and do not readily form ions or covalent bonds.

Transition Metals GCSE: Properties, Coloured Compounds and Catalysts

Typical properties

Transition metals are usually strong, dense, shiny metals with high melting points.

Coloured compounds

AQA and Edexcel questions may compare transition-metal compounds with Group 1 compounds.

Catalysts

Iron, nickel and platinum are common examples when GCSE questions ask about industrial reactions.

Trends in the Periodic Table — What to Know for the Exam

GCSE periodic table trends questions usually reward explanations, not just pattern recall. For AQA and Edexcel, the strongest answers link the trend to atomic structure, electron shells and attraction between the nucleus and electrons.

Atomic radius decreases from left to right across the same period.
Atomic radius increases from top to bottom down a group.
Group 1 reactivity increases down the group, while Group 7 reactivity decreases down the group.
Metallic character decreases as you move right and upwards across the table.

Exam explanation checklist

Name the trend clearly.
State whether the element is gaining or losing electrons.
Refer to outer-shell distance and attraction to the nucleus.
Compare Group 1 and Group 7 in opposite directions.
Use the periodic table to support the answer, not replace the explanation.

Check the official AQA GCSE Chemistry specification

Interactive quiz

Periodic Table GCSE Quiz - 30 Exam-Style Questions

Test Group 1, Group 7, Group 0, transition metals, periodic trends, Mendeleev and electronic configuration with the 30 questions below. Choose an answer to reveal the explanation.

0/30 answered · 0 correct

1/30

Score: 0/0

Which of the following best explains why the reactivity of Group 1 elements increases as the atomic number increases?

Hint

Consider the relationship between the distance of the outer shell from the nucleus and the strength of electrostatic attraction.

Mendeleev and the Periodic Table

GCSE Chemistry also expects students to know why Mendeleev’s periodic table was important. He arranged elements mainly by atomic mass but left gaps where the properties did not fit. Those gaps predicted elements that were discovered later, and their properties matched his predictions. Modern periodic tables are arranged by atomic number, which gives a more accurate pattern because atomic number is the number of protons.

AQA Periodic Table Exam Questions — Practice

Students searching for periodic table aqa gcse practice usually need the question format and the answer structure. Use these examples to rehearse what a mark scheme expects before moving into full GCSE Chemistry past papers.

Question type 1

Explain why sodium is more reactive than lithium using electronic structure.

Answer schema

Mention Group 1, one outer electron, sodium has more shells and the outer electron is lost more easily.

Question type 2

Use the periodic table to identify the group and period of an element with atomic number 16.

Answer schema

Find sulfur, then state Group 6/16 depending on table style and Period 3.

Question type 3

Predict what happens when chlorine water is added to potassium iodide solution.

Answer schema

Chlorine is more reactive than iodine, so iodine is displaced and the solution changes colour.

Periodic table GCSE quiz - 30 questions Full AQA Chemistry past papers →

Periodic Table GCSE FAQ

Is the periodic table given in AQA GCSE Chemistry?

Yes. AQA GCSE Chemistry provides a periodic table in the exam. You do not need to memorise every element, but you do need to use the table to find atomic number, groups, periods and patterns in properties.

What is Group 7 in GCSE Chemistry?

Group 7 contains the halogens, including fluorine, chlorine, bromine and iodine. They have seven outer electrons, form 1- ions and become less reactive down the group.

Why does Group 1 reactivity increase down the group?

Group 1 reactivity increases down the group because the outer electron is further from the nucleus and is shielded by more electron shells. It is lost more easily, so the metal reacts more strongly.

Why does Group 7 reactivity decrease down the group?

Group 7 reactivity decreases down the group because the outer shell is further from the nucleus. The atom attracts an extra electron less strongly, so it is less reactive.

Why are noble gases unreactive?

Noble gases are unreactive because they have full outer electron shells. They do not need to gain, lose or share electrons, so they rarely form chemical bonds.

What do periods show in the periodic table?

Periods are the horizontal rows. Elements in the same period have the same number of occupied electron shells, and atomic number increases from left to right.

What do groups show in the periodic table?

Groups are the vertical columns. Elements in the same group have the same number of outer electrons, which is why they often have similar chemical properties.

What did Mendeleev do for the periodic table?

Mendeleev arranged elements by patterns in their properties and left gaps for undiscovered elements. Later discoveries matched his predictions, which supported his periodic table.

Do I need to memorise the periodic table for GCSE?

No. A periodic table is provided in GCSE Chemistry exams, including AQA and Edexcel papers. You need to know how to use it to explain groups, periods, trends and electronic structure.

What are transition metals in GCSE Chemistry?

Transition metals are the central block of metals in the periodic table. At GCSE, they are linked with high melting points, high density, coloured compounds and use as catalysts.

Next GCSE and KS3 Chemistry Steps

GCSE Chemistry quizzes for periodic table practice GCSE atomic structure revision GCSE Chemistry past papers KS3 Periodic Table